Which of the following is NOT an assumption of the kinetic theory of ideal gases?

The kinetic energy per $g\;mol$ for a diatomic gas at room temperature is

Calculate the volume occupied by 250 moles of water vapor at STP, assuming ideal gas behavior.

Vessel $A$ is filled with hydrogen while vessel $B,$ whose volume is twice that of $A,$ is filled with the same mass of oxygen at the same temperature. The ratio of the mean kinetic energies of hydrogen and oxygen is

The relation between the gas pressure $P$ and average kinetic energy per unit volume $E$ is

The temperature at which the average translational kinetic energy of a molecule is equal to the energy gained by an electron in accelerating from rest through a potential difference of $1\;volt$ is

The average kinetic energy of hydrogen molecules at $300\;K$ is $E.$ At the same temperature, the average kinetic energy of oxygen molecules will be

If the molecular diameter of a gas is doubled, while the number density remains constant, its mean free path will:

The molecular weights of ${O_2}$ and ${N_2}$ are 32 and 28 respectively. At ${15^ \circ }C,$ the pressure of $1\;g\;{O_2}$ will be the same as that of $1\;g\;{N_2}$ in the same bottle at the temperature

The temperature of a gas is -68$^ \circ C$. At what temperature will the average kinetic energy of its molecules be twice that of at -68$^ \circ C$?

In the absence of intermolecular forces of attraction, the observed pressure $p$ will be